For which of the following reactions is AS° > 0.Choose all that apply.2NH3(g) + 3N2O(g) → 4N2(g) + 3H2O(g)2H2O(g) + 2Cl2(g) →4HCl(g) + O2(g)2NO(g) + O2(g) → 2NO2(g)NH4HS(s) → NH3(g) + H₂S(g)2NH3(g) + 202(g) → N₂O(g) + 3H2O(l)

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Answered: For which of the following reactions is…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Consider the following reaction. 2A(g)+B(g) = 4C(g) H=-107 kJ/molUnder which reaction conditions would you expect to have the greatest equilibrium yield of C(g)?
The thermodynamic values from part A will be useful as you work through part B: ΔH∘rxn 243.5kJ/mol ΔS∘rxn 172.0J/(mol⋅K) Calculate the equilibrium constant for the following reaction at room temperature, 25 ∘C BaCO3(s)→BaO(s)+CO2(g)
Use thermochemical data given in the table to decide whether the equilibrium constant for each of the following reactions will increase or decrease with temperature. Substance AH; (kJ/mol) CO(g) CO₂ (g) CS₂(g) CH₁ (9) H₂(g) H₂S(g) H₂O(g) N₂ (9) NH3 (9) O₂(g) -111 -394 117 -74.9 0 -20.5 -242 0 -45.9 0 a. CO₂(g) + H₂(g) → CO(g) + H₂O(g) O The equilibrium constant will increase with temperature increase. O The equilibrium constant will decrease with temperature increase. b. 2CO2 (g) 2CO(g) + O2(g) O The equilibrium constant will increase with temperature increase. O The equilibrium constant will decrease with temperature increase.
Which one of the following reactions cannot proceed spontaneously as written at any temperature? Assume that ΔH°rxn does not depend on temperature. A. 2Cl2O(g) → 2Cl2(g) + O2(g) ΔH°rxn = –151 kJ B. 3O2(g) → 2O3(g) ΔH°rxn = +284 kJ C. COCl2(g) → CO(g) + Cl2(g) ΔH°rxn = +112 kJ D. 2C(s) + 2S(s) + O2(g) → 2COS(g) ΔH°rxn = –137 kJ E. N2O4(g) → 2NO2(g) ΔH°rxn = +171 kJ
For the reaction: AgI(s) + 1/2Br2(g) → AgBr(s) + 1/2I2(s), ΔH° = –54.0 kJ ΔHf° for AgBr(s) = –100.4 kJ/mol ΔHf° for Br2(g) = +30.9 kJ/mol The value of ΔHf° for AgI(s) is:
Calculate the standard enthalpy change for the reaction at 25 °C. Standard enthalpy of formation values can be found in this list of thermodynamic properties. MgCl₂ (s) + H₂O(1) AH;xn= V → B MgO(s) + 2 HCl(g) MacBook Air H N M 1 9 DD $10 P m kJ
Below what temperature does the following reaction become nonspontaneous? 2 HNO3(aq) + NO(g) → 3 NO2(g) + H2O(l) ΔH = +136.5 kJ; ΔS = +287.5 J/K A) 39.2 K B) 151 K C) 475 K D) 501 K
For the following reaction, AH = 2816 kJ. 6 CO₂(g) + 6 H₂O(I) ⇒ C6H12O6(s) + 6 O₂(g) Select ONE combination of strategies that when applied to this system at equilibrium will result in an increase in the amount of C6H₁2O6 as equilibrium is re-established? a. Increasing Po₂ by adding more O2; increasing the temperature; decreasing the volume; or removing CO₂ b. Increasing Po₂ by adding more O₂ and decreasing the volume C. Decreasing the volume d. Increasing Po₂ by adding more O₂ e. Increasing the temperature
For which of the following reactions is AS° > 0. Choose all that apply. CH₂(g) + H₂O(g) → 3H₂(g) + CO(g) 2NO(g) + 2H₂(g) → N₂(g) + 2H₂O(l) 2NO(g) + O₂(g) → 2NO₂(g) 2CO₂(g) + N₂(g) → 2CO(g) + 2NO(g) ONH₂HS(s)→ NH3(g) + H₂S(g)
What is AS for the combustion of propane? C3H8(g) +502(g) → 3CO2(g) + 4H₂O(g) Substance C3H8(g) O2(g) CO2(g) H₂O(g) S(J/K mol) 269.9 205.0 213.6 188.7
The thermodynamic values from part A will be useful as you work through part B: ΔH∘rxn 243.5kJ/mol ΔS∘rxn 172.0J/(mol⋅K) Calculate the equilibrium constant for the following reaction at room temperature, 25 ∘C BaCO3(s)→BaO(s)+CO2(g)
Consider the following chemical reaction. 2CH,(g) +30,(g) – 2CO(g) + 4H,O() Select all the statements that are correct. The potential energy of the reactants is higher than the potential energy of the products. O The reactants can adopt a larger number of configurations than the products. The reaction should become more product favored at hiph temperatures. IThe reactants can adopt a fewer number of confipurations than the products. I The potential energy of he reactants is lower than the potential energy of the products. The reaction should become more product lavored at low temperatures.

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For which of the following reactions is AS° > 0. Choose all that apply. 2NH3(g) + 3N2O(g) → 4N2(g) + 3H2O(g) 2H2O(g) + 2Cl2(g) →4HCl(g) + O2(g) 2NO(g) + O2(g) → 2NO2(g) NH4HS(s) → NH3(g) + H₂S(g) 2NH3(g) + 202(g) → N₂O(g) + 3H2O(l)